Given the values of so given below in j/mol k and of δhfo given in kj/mol, calculate the value of δgo in kj for the combustion of 1 mole of methane to form carbon dioxide and gaseous water at 298 k. s (ch4(g)) = 189 s (o2(g)) = 200 s (co2(g)) = 210 s (h2o(g)) = 186 δhfo (ch4(g)) = -75 δhfo (co2(g)) = -396 δhfo (h2o(g)) = -220

-759 kJ

Explanation:

The reaction is

CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g)

And, ΔG° = ΔH° - TΔS°

Where T is the temperature in K.

ΔH° = ∑n*H°f, reactants - ∑n*H°f, products

Where n is the number of moles in the stoichiometry reaction. H°f,O₂(g) = 0 because it's a substance formed by only one element.

ΔH° = [2*(-220) +(-396)] - [-75] = -761 kJ

ΔS° = ∑n*S°, reactants - ∑n*S°, products

ΔS° = [2*(186) + 210] - [2*200 + 189] = -7 J/K = -0.007 kJ/K

So

ΔG° = -761 - 298*(-0.007)

ΔG° = -759 kJ

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a saline water is fed to a reverse osmosis unit at flow rate o rotameter connected to reject (retentate) line reads 8 installed in reject and permeate line reads 15.2 milli siemens/cm and 300 micro siemens/com respectively.